Match the appropriate tests with the indicated procedure form the table above. Ceric Sodium Ferric Acetyl Sodium Acetate Ester Lucas Ammonium Metal Chloride Chloride Fusion Test Test Test Nitrate Test Test Test Test A
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Q: The decomposition of ammonia on a platinum surface at 856 °C NH3 1/2 N2 + 3/2 H2 is zero order in…
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Q: How many hydrogen atoms are in a 12.2 g sample of ammonia?
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Q: 28 Which is more acidic, a beer with [H,0*)= 3.16 × 10-5 or a wine with [H,O'] = 5.01 x 10 4? %3D
A: Value of pH tells the acidity of solution. Lesser the value of pH, more is the acidity.
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A: Volume of LiOH solution = 2.75 L Molarity = 0.575 M
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Q: 1. 20.0 ml of 0.500 M Acetic Acid (CH3COOH) is titrated with 0.500 M KOH. Find the pH a. Before…
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- Solutions of cobalt (II) ions have a magenta color with a molar absorptivity constant (e) value at 511 nm of 5.87 M-1cm-1. A 0.500 mL sample is transferred from a 50.0 mL stock solution of Co(NO3)2 and diluted with water to a final volume of 7.50 mL. The dilution had an absorbance value at 511 nm in a standard cuvette (1.00 cm light path) of 0.382. Calculate the mass of Co(NO3)2 contained in the original 50.0 mL stock solution.A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.A 10.00mL sample of alcoholic ethyl acetate was diluted to 100.00 mL. 20.00 mL was aliquoted and mixed with 40.00 mL of 0.04672 M KOH. The resulting mixture was heated for 2 hours. CH3COOC2H5 + OH- → CH3COO- + C2H5OH After cooling, the excess OH was back titrated with 3.41 mL of 0.05042 M H2SO4. Answer the following: Calculate the number of moles of OH- that reacted with ethyl acetate. Calculate the number of moles of ethyl acetate in the 20.00 mL solution. What is the mass of ethyl acetate (FW=88.11 g/mol) in the original 10.00 mL sample?
- Preparation of cpper(1) chloride What color observed for the solution of Na2SO3 in water? What colour observed for solutions of CuCl2.2H2O in water? Which ion is responsible for the colour that is observed in the CuCl2 solution? What is observed when th Na2SO3 solution is added to the CuCl2? Which gas can be smelled when H2SO4 is added to the mixture? What is the colour of the CuCl when it is filtered on Buchner funnel? (before it is exposed to the atmosphere)Preparation of cpper(1) chloride What color observed for the solution of Na2SO3 in water? What colour observed for solutions of CuCl2.2H2O in water? Which ion is responsible for the colour that is observed in the CuCl2 solution? What is observed when th Na2SO3 solution is added to the CuCl2? Which gas can be smelled when H2SO4 is added to the mixture? What is the colour of the CuCl when it is filtered on Buchner funnel? (before it is exposed to the atmosphere) What is the colour of the CuCl when it is filterd on the Bucher funnel? (before it is exposed to the atmosphere) Does the colour of the CuCl remain the same if you leave it to dry in the atmosphere? Calculate the percentage yields for the experimentA sample is analyzed for chloride by the Volhard method. Calculate the %KCl from the following data: Wt of sample = 0.5000g; Vol of AgNO3 added = 35.00ml; M of AgNO3 = 0.1157; Vol of SCN- used for back titration = 14.71ml; M of SCN- = 0.08598; Atomic wts: Ag = 107.87, N = 14.00, Cl = 35.5, O = 16.00
- A 50.00mL sample with BaCl2 was diluted to 650 mL. Aliquots of 100.00 mL of this solution were analysed using Mohr and Volhard methods. The following data were obtained. Volhard method: Volume of AgNO3 = 100mL; Volume of KSCN = 18.25mL Mohr Method: volume of AgNO3: sample = 27.80mL (blank) = 0.30mLWhat is the %BaCl2 using Mohr and Volhard Method. Concentration of KSCN: 0.04000M Concentration of AgNO3: 0.03000MH1 gramof Sampleof an impure mixture af NARCOZ and Natteo, containing impurties is dissalved and tityated with SN Hel wit p colourless after addition5mD otacid-Methyt ge is then added and 22ontof, acid reguired orange tochange the of Naz coz benotphthalein as indicator, the sotudion Curns this indicator what is the percoulye and Na Heoz in the sample ?A Sample Containfng mmol of KNOS is "parsed 6.00 x10-2² mmol of vesay ad z.00x102 mmol af ves@y ad 2.00x1o2 though a cation -excharye Column. the Colculate. volume o.02.00 M NaH of needed to titrete the elwate,
- A sample of Al;(SO.); weighing 7.52-g was dissolved in enough water and diluted to 250.0-mL. 100.0-mL of the dilution was transferred to another flask, 10.0-mL of 0.050M EDTA, 20-ml of buffer solution, 50-mL of alcohol and 2.0-ml dithizone TS were added. The resulting solution required 8.7-mL of 0.031M ZnSO, to reach the endpoint. (Note: Each ml of 0.050M EDTA is equivalent to 16.66-mg Al:(SO.);•18H;0). Compute for the percent purity of the sample.Finely ground mineral (0.9315 g) was dissolved in 25 mL of boiling 4 M HCl and diluted with 175 mL H2O containing two drops of methyl red indicator. The solution was heated to 100C, and 50 mL of warm solution containing 2.0 g (NH4)2C2O4 were slowly added to precipitate CaC2O4. Then 6 M NH3 was added until the indicator changed from red to yellow, showing that the liquid was neutral or slightly basic. After slow cooling for 1 h, the liquid was decanted and the solid transferred to a filter crucible and washed with cold 0.1 wt% (NH4)2C2O4 solution five times until no Cl- was detected in the filtrate upon addition of AgNO3 solution. The crucible was dried at 105C for 1 h and then at 500 ± 25 C in a furnace for 2 h. Ca2+ + C2O42- --> CaC2O4.H2O(s) -->500C CaCO3(s) The mass of the empty crucible was 16.9743 g, and the mass of the crucible with CaCO3(s) was 17.198164 g. Find the wt% Ca in the mineral. a) Why is the unknown solution heated to boiling and the precipitant solution,…You are assigned an unknown solution that contains Group III cations. To -1 mL of this solution was added 6 M NH3 the solution was agitated to mix well, and a reddish-brown precipitate with a gelatinous solid clinging to the inner walls of the test tube was observed. The solution was centrifuged and the supernatant was tested for completeness of precipitation by adding an additional drop of 6 M NH3. No cloudiness was observed as the drop of reagent diffused through the solution. The supernatant was then carefully decanted into a clean test tube, labeled (1st solution), and saved for further testing later. The precipitate remaining in the test tube was washed with a small amount of water, centrifuged, and the wash decanted and discarded. To the precipitate was added about 10 drops of 6 M NAOH plus ~1 mL H20 and the test tube was vigorously agitated. The resulting suspension was centrifuged and the supernatant liquid was transferred to another clean test tube and clearly labeled (2nd…